Answer:
2:3
You'd need 33.3 moles of potassium chlorate, KClO3 , to produce that much oxygen. Notice that you have a 2:3. mole ratio between potassium chlorate and oxygen gas, which means that, regardless of how many moles of the former react, you'll always produce 3/2 times more moles of the latter.
Explanation:
Answer:Mass of Potassium chloride =1.762g
Explanation:
Mass of empty beaker = 23.100 g
Mass of beaker with Potassium chloride = 24.862g
Mass of Potassium chloride = Final weight - initial weight = Mass of beaker with Potassium chloride - Mass of empty beaker = 24.862-23.100 = 1.762g
Answer:
N-ethyl-2-methylpropan-2-amine
Explanation:
In this case, we have to start with the <u>IR info</u>. The signal on 3400 cm^-1 indicates the presence of a <u>hydrogen bonded to the heteroatom</u>. In this case, we have nitrogen in the formula, so we will have the <u>amine group</u>.
On the other hand, we have to analyze the NMR info:
a) We have 2 singlets => This indicates the presence of 2 different hydrogens without neighbors.
b) We have a triplet => This indicates the presence of <u>CH3 bonded to a CH2</u>.
c) We have a quartet => This indicates the presence of <u>CH2 bonded to a CH3</u>.
From b) and c) we can conclude that we have the <u>ethyl group</u> bonded to a nitrogen.
Finally, we have to add 4 more carbons in such a way that we only have a single signal. In this case the <u>ter-butyl group</u>.
In that way, we will have <u>2 singlets</u> (from the CH3 groups in the ter-butyl and the H on the N). Also, we will have the <u>quartet </u>on the CH2 in the ethyl group and the <u>triplet</u> on the CH3 in the ethyl group
Answer:
- Add AgNO₃ solution to both unlabeled flasks: based on solubility rules, you can predict that when you add AgNO₃ to the NaCl solution, you will obtain AgCl precipitate, while no precipitate will be formed from the NaClO₃ solution.
Explanation:
<u>1. Adding AgNO₃ to NaCl solution:</u>
- AgNO₃ (aq) + NaCl (aq) → AgCl (s) + NaNO₃ (aq)
<u>2. Adding AgNO₃ to NaClO₃ solution</u>
- AgNO₃ (aq) + NaClO₃ (aq) → AgClO₃ (aq) + NaNO₃ (aq)
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<u>3. Relevant solubility rules for the problem.</u>
- Although most salts containing Cl⁻ are soluble, AgCl is a remarkable exception and is insoluble.
- All chlorates are soluble, so AgClO₃ is soluble.
- Salts containing nitrate ion (NO₃⁻) are generally soluble and NaNO₃ is not an exception to this rule. In fact, NaNO₃ is very well known to be soluble.
Hence, when you add AgNO₃ to the NaCl solution the AgCl formed will precipitate, and when you add the same salt (AgNO₃) to the AgClO₃ solution both formed salts AgClO₃ and NaNO₃ are soluble.
Then, the precipiate will permit to conclude which flask contains AgCl.
Answer:
No one is reduced.
Explanation:
It is an example oxidation reaction in which carbon is oxidised to form carbon dioxide.
